1. Unit 1: Atoms, Elements, and Compounds
Grade 9 Science
Unit 1: Atoms, Elements, and Compounds

2. Grade 9 Science... Unit 1
Chapter 1: Atomic theory explains the composition and behaviour of matter.

3. Lab Safety... A Review
Safety rules and procedures MUST be your top priority.
Know them before you do the lab and use them while doing the lab.

4. Complete activity 1-1A pg. 9
Laboratory Safety
Complete activity 1-1A pg. 9

5. Safety Rules for the Science Lab pages 10-11
General
Glassware
Chemicals
Hot plates and open flames
Electrical equipment

6. W workplace H hazardous M materials I information S system
WHMIS... Page 12
W workplace H hazardous M materials I information S system

8. Hazard Symbols... Page 13
Dangerous Container
Dangerous Contents

9. Properties of Matter Matter is anything that has mass and volume.
Mass is the amount of matter in a substance or object.
Volume is the amount of space a substance or object occupies.

10. Matter is made up of elements.
Elements are substances that contain one type of matter and cannot be broken down or separated into simpler substances.

12. Characteristics of matter that are often observed or measured.
Describing Matter
1. Physical Properties pg. 18
Characteristics of matter that are often observed or measured.
Can be either qualitative (observed) or quantitative (measured).

13. Color
Malleability
Lustre
Conductivity
Boiling point
Melting point
Texture
Magnetism
Density

14. Determines a substances usefulness.
2. Chemical Properties pg. 19
Observed when substances react with each other.
Determines a substances usefulness.

15. Reactivity
Combustibility

16. Core Lab Activity 1-2C pg. 20
Physical and Chemical Properties

17. Theory vs. Law A law is better supported than a theory.
Most laws are supported by different and robust experimental evidence.
Theories can change or be modified
Laws rarely change

18. Atomic Theory

19. Atomic Theory The descriptions of matter and how it behaves.
Has undergone many modifications as new facts became available.

20. An atom consists of a
nucleus
(of protons and neutrons)
electrons in space about the nucleus

21. The Atom

22. Inside the Atom Subatomic Particle Charge Mass Location Proton (p+) +
Large
Nucleus
Neutron (n)
neutral
Electron(e-) -
Very small
Energy levels

23. Early ideas years ago
Empedocles: matter was composed of four “elements”; earth, air, wind, and fire.

24. 460 BC
Democritus: eventually a substance will be cut into a piece that can no longer be cut.
He called this piece atomos.

25. All matter was composed of four elements Earth, air, water and fire
Aristotle
All matter was composed of four elements
Earth, air, water and fire

26. Development of Atomic Theory
John Dalton
He suggested that the particles that make up matter are like small, hard spheres that are different for different elements.
He defined an atom as the smallest particle of an element.

27. Dalton’s Model... Billiard Ball Model

28. J.J. Thomson
He suggested that all atoms must contain electrons (negative charge).
His model pictured a positively charged ball with the negatively charged electrons embedded in it.

29. Thomson’s Model... Raisin Bun Model

30. Ernst Rutherford
He discovered that atoms have a nucleus.
There are two kinds of particles in the nucleus; protons (positive charge) and neutrons (neutral).

31. Rutherford’s Model... Planetary Model

32. Rutherford was able to develop Thomson’s model due to the development of new technologies. (gold foil experiment)
The development of cyclotrons and proton accelerators have further developed the model accepted today.

33. Rutherford’s Experiment
they fired Helium nuclei at a piece of gold foil which was only a few atoms thick.
Gold foil
They found that while most of the helium nuclei passed through the foil, a small number were deflected and, to their surprise, some helium nuclei bounced straight back.
Helium nuclei

34. However, this was not the end of the story.
Rutherford’s new evidence allowed him to propose a more detailed model with a central nucleus.
He suggested that the positive charge was all in a central nucleus. With this holding the electrons in place by electrical attraction
However, this was not the end of the story.

35. Niels Bohr
He proposed that electrons surround the nucleus in specific energy levels or shells.
Each electron has a particular amount of energy.

36. Bohr’s Model... Orbital Model

37. Summary...